The following values are the only energy levels of a hypothetical one-electron atom:
E₆ = -2×10⁻¹⁹J E₅ = -7×10⁻¹⁹J
E₄ = -11 ×10⁻¹⁹J E₃ = -15 ×10⁻¹⁹J
E₂ = -17 ×10⁻¹⁹J E₁ = -20×10⁻¹⁹J
(a) If the electron were in the n = 3 level, what would be the highest frequency (and minimum wavelength) of radiation that could be emitted?

In this electronic setup, there won't be any energy development from n=3 to n=1 since all electronic stages below n=3 contain energy that is almost equal.

When the excited electron transitions back to a lower electron orbital, emission takes place.
The radiation that is emitted is known as luminescence. At energies equal to or lower than the energy corresponding to the absorbed radiation, luminescence can be seen.
After initial absorption, one of two pathways can lead to emission.

Alpha particles, beta particles, and gamma rays are the three most prevalent forms of radiation.

It can be created artificially or by unstable atoms that experience radioactive decay.
From its source, radiation spreads outward as energetic waves or particles. Radiation comes in a variety of forms, each with its own characteristics and impacts.

Learn more about radiation here:

https://brainly.com/question/4072364

#SPJ4